Problem: Elemental phosphorus occurs as tetratomic molecules, P4. What mass (g) of chlorine gas is needed to react completely with 455 g of phosphorus to form phosphorus pentachloride?

FREE Expert Solution

We will begin solving this problem by analyzing what information we have, to solve this problem: 

Firstly, we will need to write a balanced equation for the data provided.

Phosphorous P4 reacts with Chlorine gas to form Phosphorous Pentachloride

Recall that, Chlorine gas - Cl2 exists as a diatomic molecule and the prefix -penta refers to 5 therefore, we can say that the following reaction takes place  

P4 (s) + Cl2 (g) → PCl5 (s)

  • Write down the number of atoms on the left side and the right side separately.
  • There are 4 P and 2 Cl on the left and 1 P and 5 Cl on the right.
  • Multiply PCl5  by 4 to have an equal number of P’s (4 and 4, therefore, they are equal).
  • Finally, there are 20 Cl on the right side and only 2 on the left. Multiply Clby 10. Now both sides have an equal number of atoms.
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Problem Details

Elemental phosphorus occurs as tetratomic molecules, P4. What mass (g) of chlorine gas is needed to react completely with 455 g of phosphorus to form phosphorus pentachloride?

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Our tutors have indicated that to solve this problem you will need to apply the Stoichiometry concept. You can view video lessons to learn Stoichiometry. Or if you need more Stoichiometry practice, you can also practice Stoichiometry practice problems.

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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.